Quick questions on Enthalpy of neutralisation and calorimetry explained: HSC Chemistry Module 6

4short Q&A pairs drawn directly from our worked dot-point answer. For full context and worked exam questions, read the parent dot-point page.

What is sources of error?

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To reduce these errors, use a stirred, insulated calorimeter, a graphed temperature-time correction, and equal initial temperatures for the two reactants.

What is q1?

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Define the enthalpy of neutralisation and state its standard value for a strong acid and strong base. [2 marks]

What is q2?

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50.0 mL of 0.500 mol L

^{-1}

HCl is mixed with 50.0 mL of 0.500 mol L

^{-1}

NaOH. The temperature rises by 3.40 degrees C. Calculate

\Delta H

of neutralisation.

What is q3?

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Account for the following observations: (a) the enthalpy of neutralisation for HF + NaOH is

-68

kJ mol

^{-1}

, more exothermic than the strong-strong value. (b) The enthalpy for

CH_3COOH

+ NaOH is

-55

kJ mol

^{-1}

, less exothermic than the strong-strong value. (c) State one source of error in a polystyrene-cup calorimeter.

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